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3 years ago

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PLS HELP!I will give brainliest! When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of th

e products is 590 kJ/mol. The equation is shown.
H2 + I2 → 2HI

What is the total energy of the reaction? Is this an endothermic or exothermic reaction?
A. –9 kJ/mol, exothermic
B.9 kJ/mol, exothermic
C. 9 kJ/mol, endothermic
D. –9 kJ/mol, endothermic

1 answer:

Veronika [31]3 years ago

4 0

Answer:

Here, we are required to determine the total energy of the reaction and determine if the reaction is an endothermic or exothermic reaction.

The correct answer is option C.

First, we need to determine the energy of the reaction.

The energy of the reaction is the change in enthalpy between the product and reactants.

Change of Enthalpy,

Hreaction = Hproduct - Hreactant.

Therefore, for the reaction above, the change in enthalpy is:

Hreaction = 590kJ/mol - 581kJ/mol.

Hreaction = 9kJ/mol.

Hence, since the reaction has an enthalpy change of 9kJ/mol, the reaction is endothermic (i.e energy is absorbed).

Explanation:

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3 years ago

In the equation CH4 + 2O2 --> 2H2O + CO2 What is the mass of CO2 produced when 35g of O2 reacts?

Anestetic [448]

Answer:

24.06 g of CO₂

Explanation:

The balanced equation for the reaction is given below:

CH₄ + 2O₂ —> 2H₂O + CO₂

Next, we shall determine the mass of O₂ that reacted and the mass of CO₂ produced from the balanced equation. This can be obtained as follow:

Molar mass of O₂ = 2 × 16 = 32 g/mol

Mass of O₂ from the balanced equation = 2 × 32 = 64 g

Molar mass of CO₂ = 12 + (2×16)

= 12 + 32

= 44 g/mol

Mass of CO₂ from the balanced equation = 1 × 44 = 44 g

SUMMARY:

From the balanced equation above,

64 g of O₂ reacted to produce 44 g of CO₂.

Finally, we shall determine the mass of CO₂ produced by the reaction of 35 g of O₂. This can be obtained as follow:

From the balanced equation above,

64 g of O₂ reacted to produce 44 g of CO₂.

Therefore, 35 g of O₂ will react to produce = (35 × 44)/64 = 24.06 g of CO₂.

Thus, 24.06 g of CO₂ were produced from the reaction.

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2 years ago

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Explanation:

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3 years ago

How many moles in 3.69 x 10^30 molecules of carbon dioxide?

Sedaia [141]

$0.612 \times 10^{7} \text { moles of } \mathrm{CO}_{2}$ are present in $3.69 \times 10^{30} \text { molecules of } \mathrm{CO}_{2}$

<u>Explanation:</u>

It is known that each mole of an element is composed of avagadro's number of molecules. So if we need to determine, we need to divide the number of molecules with the avagadro's number.

So,

$1 mol of element =6.02 \times 10^{23} molecules of element$

As here $3.69 \times 10^{30}$ molecules of carbon di oxide is given. So the moles in it will be

No. of moles of carbon dioxide = $\frac{3.69 \times 10^{30}}{6.02 \times 10^{23}}$

No. of moles = $0.612 \times 10^{7}$ moles of carbon dioxide.

Thus,

$0.612 \times 10^{7}$ of carbon dioxide are present in $3.69 \times 10^{30} \text { molecules of } \mathrm{CO}_{2}$ .

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